Structure and Properties Review

Chemistry Exam Review Thinking and Investigation (70) 1. Draw Lewis dot diagrams for the following ionic and covalent bonds. (5) NaCl

HCN

KCl

CCl4

CaCl

2. Sort each of the following forces from strongest to weakest: Dispersion, Dipole-Dipole, HBonding, Ion-Dipole, Ion-Ion, Covalent Bonds (3)

3. Complete the following chart (12) Example

Lewis Dot Diagram

E.N.D calculation

VSEPR structure

Shape formed

Type of compound

Reason

AlH2Cl

CH3Cl

CCl2H2

HCl

4. Write the following equations as balanced chemical equations. Include the states for each substance. (9) A) Calcium metal + hydrocyanic acid = calcium cyanide + hydrogen (3)

B) Cupric chloride hexahydrate = cupric chloride + water (3)

C) Potassium sulphate + iron (II) nitrate = iron (II) sulphate + potassium nitrate (3)

5. Name each compound: (10) decane iron (III) carbonate colbatous chloride hexahydrate tin (IV) monohydrogen hypophosphite thiocyanic acid H3AsO2 (aq) Ca3As2 (NH4)2B4O7 SF6 Ni(HSO3)3

6. Calculate the average atomic mass of substance lead, Pb, given that the relative abundance of its four isotopes below (3) Isotope

Atomic Mass (U)

Relative Abundance (%)

Lead-204

203.973

1.370

Lead-206

205.974

26.26

Lead-208

206.976

20.82

Lead-209

207.977

51.55

7. Phenyl validate is a colourless liquid that is used as a flavouring agent and odourant. It contains 74.12% carbon, 7.933% hydrogen, and 17.95% oxygen by mass. If its molar mass is 178.25g/mol, determine its molecular and empirical formula. (4)

8. Determine the number of moles of hydrogen gas in a. sample that contains 5.55 x 10^24 H atoms (2)

9. Determine the number of combat (II) chloride formula units in a sample containing 0.25g of CoCl2 (2)

10. Determine the mass of hydrogen gas produced when 6.12 mol of Mg reacts with excess hydrochloric acid (5) Mg(s) + 2HCl (aq) = H2(g) + MgCl2 (aq)

11. A student preformed an experiment to determine the percent composition of Mg in MgO, she obtained 26.45g. Determine the percent error in her experiment by determining the actual % composition first. (3)

12. Write the overall, ionic and net ionic equations and circle the following spectator ions for the following. (9) A) aqueous solutions of potassium chloride and copper (I) nitrate are mixed (3)

B) aqueous copper (II) sulfate is mixed with zinc to form zinc sulphate and copper (3)

C) aqueous solutions of calcium bromide and ammonium carbonate are mixed (3)

13. Determine the mass of Ca3(PO4)2 required to produce 250.0mL of Ca ions having a concentration of 3.45mol/L (4)

14. Copper can be removed from scrap metal by adding sulphuric acid. Soluble copper (II) sulphate is formed. The copper (II) sulphate then reacts with metallic iron in a single displacement reaction, where iron (II) sulphate is formed. To simulate this reaction, a student places 0.8755g of iron (Steel wool) in a breaker that contains 55.55mL of a 0.3750mol/L solution of copper (II) sulfate. Determine the mass of copper that is formed. The equation is given below: (limiting reactant) (5)

15. Your friend sits on a 25.0L kangaroo ball, squishing the ball so that it is only 17.5L. What is the pressure inside the ball if the outside air pressure is 100kPa? (2)yte]\